Calculate the concentrations of `H_(3)O^(+) and OH^(-)` ions in the solution with the following pH values at `25^(@)C`
(1) pH=5.0
(2) pH=12.

Explanation

(1) In case of a solution with pH=5,
`[H_(3)O^(+)]=10^(-pH)(M)=10^(-5)(M)`
`therefore` In this solution,
`[OH^(-)]=(10^(-14))/([H_(3)O^(+)])=(10^(-14))/(10^(-5))(M)=10^(-9)(M)`
(2) In case of a solution with pH=12,
`[H_(3)O^(+)]=10^(-pH)(M)=10^(-12)(M)`,
`therefore`In this solution, `[OH^(-)]=(10^(-14))/([H_(3)O^(+)])=(10^(-14))/([H_(3)O^(+)])=(10^(-14))/(10^(-12))(M)=10^(-2)(M)`.